Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

7. Gases

The Ideal Gas Law

General Chemistry

7. Gases

The Ideal Gas Law

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Multiple Choice

What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g of He and 94.6 g of CO2 at 398 K, assuming ideal gas behavior?

12.3 atm

18.4 atm

15.8 atm

9.7 atm

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Verified step by step guidance

First, calculate the number of moles of each gas using the formula: \( n = \frac{m}{M} \), where \( m \) is the mass of the gas and \( M \) is the molar mass. For helium (He), the molar mass is approximately 4.00 g/mol, and for carbon dioxide (CO2), it is approximately 44.01 g/mol.

Calculate the moles of helium: \( n_{\text{He}} = \frac{48.5 \text{ g}}{4.00 \text{ g/mol}} \).

Calculate the moles of carbon dioxide: \( n_{\text{CO2}} = \frac{94.6 \text{ g}}{44.01 \text{ g/mol}} \).

Use the ideal gas law to find the total pressure exerted by the gas mixture. The ideal gas law is given by \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the total number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.

Calculate the total moles of gas by adding the moles of helium and carbon dioxide. Then, rearrange the ideal gas law to solve for pressure: \( P = \frac{nRT}{V} \). Substitute the total moles, the given temperature (398 K), the volume (10.0 L), and the ideal gas constant into the equation to find the pressure.